[zujca]

3 NaHCO₃ + C₆H₈O₇ = C₆H₅Na₃O₇ + 3 CO₂ + 3 H₂O
This is the reaction.
I have:
m(NaHCO₃)=1g
V(C₆H₈O₇)=2ml
ρ(C₆H₈O₇)=1,66 g/ml
p=99,75 Pa
T=297 K
Now I need to calculate the volume of CO₂. I calculated that it's 210 ml, by saying that n(CO₂)=n(NaHCO₃), which is 0,0085 mol (after I calculated how much of it reacts with citric acid), then I calculated it by p·V=nRT and got 0,21l=210 ml.
I just wanted to make sure that it's correct!
Also, then I have to calculate how many does the 210 ml weigh, so I'd use the 0,0085 mol · 44 g/mol = 0,374 g.
Is all of this correct? Thank you!

[Borek]

Please list the question exactly as it is worded. The idea of using volume and density of citric acid doesn't sound right, as most likely density is that of a crystal, not that of a bulk solid.

[zujca]

Well we don't really have a question. The task was to do an experiment which has CO2 as a product and measure the volumen of CO2, calculate its mass and then calculate which molecule is in excess (in my case NaHCO3 or citric acid).
Is there another way of calculating the mass of citric acid, given the volume only, or was I supposed to measure it? It was in the liquid form as a lemon extract.

I am back, I measured the lemon extract and it's 2g.

[Borek]

OK, let's start with hydrogencarbonate. What is molar mass of NaHCO₃?

[zujca]

84 g/mol.
Also, when I did the experiment, I measured about 60 ml of CO2 in the injection + 30 ml in the tube, which is 90 ml. However with calculating from the reactants, it's supposed to be more.

[Borek]

So, how many moles of hydrogencarbonate?

And please explain how many moles of citric acid you used. First you gave density and volume of citric acid, then you gave mass of lemon extract (no idea what it is and how much citric acid it contains), and I have no idea what is what of what.